NTE Praxis: Chemistry MCQs (Practice-Test 17 of 31)
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Calculate the solubility (in M) of MgF2 (Ksp = 6.5 × 10 − 9) in water.
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Calculate the solubility (in M) of AgBr (Ksp = 5.0 × 10 − 15) in a solution that initially contains 0.25 M NaBr.
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Which of the following best describes what will happen when a solution of AgNO3 is slowly added to a saturated solution of silver acetate, CH3COOAg, without changing the volume significantly? CH3COOAg (s) ⇔ CH3COO- (aq) + Ag + (aq)
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Some of the solid silver acetate will dissolve.
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The concentration of acetate ion will increase.
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Some solid silver acetate will precipitate.
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The concentrations of acetate ion and silver ion will both increase.
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The addition of AgNO3 will have no effect on the position of the equilibrium.
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Which one of the following groups contains only salts that are expected to be soluble in water?
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ZnS, KNO3, CoS, PbCrO4
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NaCl, KNO3, Zn (NO3) 2, MgSO4
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Ca3 (PO4) 2, Cr (OH) 3, NaCl, ZnS
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AgOH, Cu (OH) 2, KCl, NaI
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A correct response is not given.
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Which of the following groups contains only salts that are expected to be highly soluble in water?
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NaCl, KNO3, ZnS, PbCrO4
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NaCl, KNO3, Zn (NO3) 2, Na2S.
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ZnS, PbCrO4, Ca3 (PO4) 2, Cr (OH) 3
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ZnS, KNO3, PbCrO4, CoS.
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A correct response is not given.
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Which of the following groups contains only salts that are expected to be slightly soluble or insoluble in water?
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NaCl, KNO3, ZnS, PbCrO4
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NaCl, KNO3, Zn (NO3) 2, Na2S.
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ZnS, PbCrO4, Ca3 (PO4) 2, Cr (OH) 3
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ZnS, KNO3, PbCrO4, CoS.
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A correct response is not given.
Use the following reaction to answer the next four questions:
Ca3 (PO4) 2 ⇔ 3 Ca2 + + 2 PO43-
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What is the correct expression for the solubility product constant for calcium phosphate?
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Ksp = [Ca2 + ] [PO43-]
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Ksp = [Ca2 + ]2 [PO43-]2
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Ksp = [Ca2 + ]2 [PO43-]2
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Ksp = [Ca2 + ]3 [PO43-]2
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The correct response is not given.
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What is the correct relationship between the solubility of calcium phosphate in pure water, C0 (Ca3 (PO4) 2), and the equilibrium concentration of calcium ion, [Ca2 + ]?
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[Ca2 + ] = 3C0 (Ca3 (PO4) 2)
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[Ca2 + ] = 2C0 (Ca3 (PO4) 2)
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[Ca2 + ] = (⅓) C0 (Ca3 (PO4) 2)
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[Ca2 + ] = (3/2) C0 (Ca3 (PO4) 2)
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The correct response is not given.
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Addition of calcium nitrate (Ca (NO3), 2), to a saturated solution of calcium phosphate would:
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have no effect on the solubility of calcium phosphate.
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cause the solubility of calcium phosphate to decrease.
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cause the solubility of calcium phosphate to increase.
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cause unpredictable changes in the solubility of calcium phosphate.
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The correct response is not given.
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Recognizing that the phosphate ion is a strong Bronsted base, we can accurately predict that addition of hydrochloric acid to a saturated solution of calcium phosphate would:
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have no effect on the solubility of calcium phosphate.
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cause the solubility of calcium phosphate to decrease.
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cause the solubility of calcium phosphate to increase.
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cause unpredictable changes in the solubility of calcium phosphate.
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The correct response is not given.
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The solubility of silver sulfate (Ag2SO4 ⇔ 2 Ag + + SO42-) in pure water is 0.0152 mol/L. Calculate the solubility product constant, Ksp, for silver sulfate.
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The solubility product constant for lead chloride (PbCl2 ⇔ Pb2 + + 2 Cl-) is Ksp = 1.6 × 10 − 5. Calculate the molar solubility of lead chloride in pure water.
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Calculate the molar solubility of gold chloride (AuCl3, Ksp = 3.2 × 10 − 25) in a solution containing 1.0 × 10 − 5 M chloride ion.
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Calculate the molar solubility of manganese hydroxide (Mn (OH) 2, Ksp = 2.0 × 10 − 13) in a solution buffered at pH = 9.00.
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What happens to the concentration of the Pb2 + and SO42-ions in a saturated solution of PbSO4 in contact with solid PbSO4 when the solution evaporates to half of its original volume?
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The concentrations of Pb2 + and SO42-increase.
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The concentrations of Pb2 + and SO42-decrease.
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The concentrations of Pb2 + and SO42-remain the same.
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It is impossible to say unless we know the Ksp of PbSO4.
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